Question

a student dissolves 12.3 g of sodium hydroxide (naoh) in 300. g of water in a well - insulated open cup. she then observes the temperature of the water rise from 20.0°c to 30.3°c over the course of 6.7 minutes.
use this data, and any information you need from the aleks data resource, to answer the questions below about this reaction:
naoh(s)→na+(aq)+oh−(aq)
you can make any reasonable assumptions about the physical properties of the solution. be sure answers you calculate using measured data are rounded to the correct number of significant digits.
note for advanced students: its possible the student did not do the experiment carefully, and the values you calculate may not be the same as the known and published values for this reaction.
is this reaction exothermic, endothermic, or neither? exothermic endothermic neither
if you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in this case. □kj
calculate the reaction enthalpy δhrxn per mole of naoh. □kj/mol

Explanation:

Step1: Determine the type of reaction

Since the temperature of the water rises, heat is released by the reaction. So the reaction is exothermic.

Step2: Calculate the heat released ($q$)

We use the formula $q = mc\Delta T$. Assume the specific - heat capacity of the solution $c = 4.18\space J/(g\cdot^{\circ}C)$ (similar to water), $m=(12.3 + 300)\space g=312.3\space g$, $\Delta T=(30.3 - 20.0)^{\circ}C = 10.3^{\circ}C$.

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Step3: Calculate the moles of $NaOH$

The molar mass of $NaOH$ is $M = 40.0\space g/mol$. The number of moles of $NaOH$, $n=\frac{m}{M}$, where $m = 12.3\space g$.

$$n=\frac{12.3\space g}{40.0\space g/mol}=0.3075\space mol$$

Step4: Calculate the reaction enthalpy $\Delta H_{rxn}$ per mole of $NaOH$

Since the reaction is exothermic, $\Delta H_{rxn}=-\frac{q}{n}$. Substitute $q = 13.4\space kJ$ and $n = 0.3075\space mol$.

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Answer:

1. exothermic
2. $13.4\space kJ$
3. $-43.6\space\frac{kJ}{mol}$